HSPS #2 SPS1a,b,c

A neutral sodium atom has 11 protons and 11 electrons, while a sodium ion has 11 protons and 10 electrons.

A neutral sodium atom has 11 protons and 10 electrons, while a sodium ion has 11 protons and 11 electrons.

A neutral sodium atom has 10 protons and 11 electrons, while a sodium ion has 11 protons and 10 electrons.

A neutral sodium atom has 11 protons and 12 electrons, while a sodium ion has 11 protons and 11 electrons.

Elements in the same period have the same number of valence electrons and similar chemical behavior.

Elements in the same group have the same number of valence electrons and similar chemical behavior.

Elements with higher atomic numbers always have more valence electrons than those with lower atomic numbers.

Elements in different groups always have different atomic masses but the same number of valence electrons.

Francium will be a nonmetal that forms negative ions because it is in the first group of the periodic table.

Astatine will be a metalloid with properties between metals and nonmetals because it is in the halogen group.

Cesium will be a highly reactive metal that readily loses one electron to form positive ions.

Radon will be a reactive gas that easily forms compounds because it is in the noble gas group.

Isotopes have different numbers of protons but the same number of neutrons in their nuclei.

Isotopes have different numbers of electrons but the same number of protons in their nuclei.

Isotopes have different numbers of neutrons but the same number of protons in their nuclei.

Isotopes have different numbers of protons and neutrons but the same number of electrons.

Metals are found on the right side, nonmetals on the left side, and metalloids in the center of the periodic table.

Metals are found on the left side, nonmetals on the right side, and metalloids along the diagonal staircase.

Metals are found only in the top rows, nonmetals in the bottom rows, and metalloids in the middle rows.

Metals are found in groups 1-10, nonmetals in groups 11-18, and metalloids are not present on the periodic table.

All elements in Period 2 will be gases at room temperature because they have low atomic masses.

All elements in Group 17 will be solids at room temperature because they are highly reactive nonmetals.

Elements with higher atomic numbers in the same group will generally have higher melting and boiling points.

All metal elements will be liquids at room temperature because metals conduct heat and electricity well.

Protons (+) and neutrons (0) in the nucleus, with electrons (+) orbiting around the nucleus.

Protons (+) and electrons (-) in the nucleus, with neutrons (0) orbiting around the nucleus.

Protons (+) and neutrons (0) in the nucleus, with electrons (-) orbiting around the nucleus.

Neutrons (0) and electrons (-) in the nucleus, with protons (+) orbiting around the nucleus.

Group 1 elements form 2+ ions because they have two valence electrons to lose.

Group 17 elements form 1- ions because they need one electron to complete their outer shell.

Group 2 elements form 1+ ions because they have one electron in their outermost energy level.

Group 16 elements form 3+ ions because they have three electrons to gain for stability.

All three have 6 protons and 6 electrons, but ¹³C has one extra neutron compared to the others.

¹²C and ¹³C both have 6 protons and 6 electrons, while C⁴⁺ has 6 protons and 2 electrons.

All three have different numbers of protons, which explains their different atomic masses and charges.

¹²C has 6 protons and 6 neutrons, ¹³C has 7 protons and 6 neutrons, and C⁴⁺ has 6 protons and 10 electrons.

Elements with fewer valence electrons always form positive ions, while those with more form negative ions.

The number of electrons lost or gained is directly equal to the number of valence electrons present.

Elements tend to lose or gain electrons to achieve a stable electron configuration similar to noble gases.

The periodic table position determines ion charge, but valence electrons have no relationship to ion formation.

It will be a nonmetal gas because it has a high atomic number and will be located on the right side.

It will be a highly reactive metal that forms 1+ ions because it would be in Group 1 below francium.

It will be a metalloid with intermediate properties because elements with high atomic numbers are always metalloids.

Its properties cannot be predicted because it has not been discovered yet and the periodic table cannot predict new elements.

They are both chlorine because they have the same number of protons, and the mass difference comes from neutrons.

They are both chlorine because they have the same number of electrons, and the mass difference is due to energy levels.

They are both chlorine because they have the same atomic mass, and the numbers 35 and 37 refer to different properties.

They are both chlorine because they have the same number of neutrons, and the mass difference comes from protons.

Metalloids are randomly distributed on the periodic table and have no predictable pattern in their properties.

Metalloids are found along the diagonal boundary between metals and nonmetals and have intermediate properties.

Metalloids are all located in the same group and have identical chemical and physical properties.

Metalloids are found only in Period 4 and their properties are completely different from metals and nonmetals.

Element X will be a reactive metal that conducts electricity well because it has a high atomic number.

Element X will be a halogen that forms 1- ions and exists as a solid at room temperature.

Element X will be a noble gas that is unreactive because elements with high atomic numbers are stable.

Element X will be a metalloid with semiconductor properties because it is located between metals and nonmetals.

All three particles have the same number of electrons and protons, but different numbers of neutrons.

²³Na and ²³Mg have the same nuclear composition because they both have 23 as their mass number.

²³Na⁺ (10 electrons) and ²³Mg (12 electrons, but 2+ ion would have 10) have same electron count but different nuclei.

Different elements cannot be isotopes of each other; isotopes must be the same element.